What mass of iron II sulfate can be obtained by reacting iron with 400 ml of 25% sulfuric acid solution (p = 1.14 g / ml)

1. Let’s write down the reaction equation:
Fe + H2SO4 = FeSO4 + H2.
2. Find the amount of sulfuric acid:
m (solution) = V (solution) * ρ (solution) = 400 ml * 1.14 g / ml = 456 g.
m (H2SO4) = (m (solution) * ω (H2SO4)) / 100% = 456 g * 25% / 100% = 114 g.
n (H2SO4) = m (H2SO4) / M (H2SO4) = 114 g / 98 g / mol = 1.16 mol.
3. According to the reaction equation, we find the amount of iron sulfate, and then its mass:
n (FeSO4) = n (H2SO4) = 1.16 mol.
m (FeSO4) = n (FeSO4) * M (FeSO4) = 1.16 mol * 152 g / mol = 176.8 g.
Answer: m (FeSO4) = 176.8 g.